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shusha [124]
2 years ago
11

Complete combustion of a sample of a hydrocarbon on excess oxygen produces equimolar quantities of carbon dioxide and water. Whi

ch of the following could be the molecular formula of the compound?
A. C2H2
B.C2H6
C.C4H8
D.C6H6
Chemistry
1 answer:
Bond [772]2 years ago
6 0
<span>C. C4H8 Given that the number of moles of CO2 and H2O produced from the combustion are equal, that means for every carbon atom, there are 2 hydrogen atoms because CO2 has only 1 carbon atom and H2O has 2 hydrogen atoms. So let's look at the available choices and see which one is correct. A. C2H2 This is a 1 to 1 ratio of carbon to hydrogen. Wrong answer. B. C2H6 This is a 1 to 3 ratio of carbon to hydrogen. Wrong answer. C. C4H8 This is a 1 to 2 ratio of carbon to hydrogen. Correct answer. D. C6H6 This is a 1 to 1 ratio of carbon to hydrogen. Wrong answer.</span>
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A sample of iron is put into a calorimeter (see sketch at right) that contains of water. The iron sample starts off at and the t
Mariulka [41]

Answer:

Therefore, the specific heat capacity of the iron is 0.567J/g.°C.

<em>Note: The question is incomplete. The complete question is given as follows:</em>

<em>A 59.1 g sample of iron is put into a calorimeter (see sketch attached) that contains 100.0 g of water. The iron sample starts off at 85.0 °C and the temperature of the water starts off at 23.0 °C. When the temperature of the water stops changing it's 27.6 °C. The pressure remains constant at 1 atm. </em>

<em> Calculate the specific heat capacity of iron according to this experiment. Be sure your answer is rounded to the correct number of significant digits</em>

Explanation:

Using the formula of heat, Q = mc∆T  

where Q = heat energy (Joules, J), m = mass of a substance (g)

c = specific heat capacity (J/g∙°C), ∆T = change in temperature (°C)

When the hot iron is placed in the water, the temperature of the iron and water attains equilibrium when the temperature stops changing at 27.6 °C. Since it is assumed that heat exchange occurs only between the iron metal and water; Heat lost by Iron = Heat gained by water

mass of iron  = 59.1 g, c = ?, Tinitial = 85.0 °C, Tfinal = 27.6 °C

∆T = 85.0 °C - 27.6 °C = 57.4 °C

mass of water = 100.0 g, c = 4.184 J/g∙°C, Tinitial = 23.0 °C, Tfinal = 27.6 °C

∆T = 27.6°C - 23.0°C = 4.6 °C

Substituting the values above in the equation; Heat lost by Iron = Heat gained by water

59.1 g * c * 57.4 °C  = 100.0 g * 4.184 J/g.°C * 4.6 °C

c = 0.567 J/g.°C

Therefore, the specific heat capacity of the iron is 0.567 J/g.°C.

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